First law of thermodynamics states what?

Answer 1

The first law of thermodynamics states that the energy of the universe is constant. In other words, energy is never created or destroyed (conservation of energy). However, this simply states the total energy of a system is constant. This quanta of energy can still be changed into various forms (potential, kinetic, thermal, etc.) through physical and/or chemical processes.

To clarify this, we will look at a very fundamental example: an apple falling on Newton's head. When the apple falls from the tree, its initial potential energy is converted to kinetic energy (it's in movement since it's falling), which is then transferred to the surrounding air atoms and Newton's head.

Now, when applying this same notion to a thermodynamic process, we can write it as a mathematical equation:

Change in internal energy=q-w

where q=heat added to the system by its surroundings and w=work done by the system on its surroundings. The idea is relatively

How exactly did we get this equation? The idea is really quite simple. The first law renders that energy cannot simply be "lost along the way"--it has to do something. Thus, when energy (in the form of heat) is added to a thermodynamic process, two things can happen: a change in internal energy or work.

Answer 2

Energy can not be created or destroyed it gets transformed

Answer 3

. As work is performed on the planet Earth, excess energy is lost in the form of

Answer 4

The First Law of Thermodynamics is the Law of Conservation of Energy - in other words, the total amount of energy in a closed system remains constant.

Answer 5

The conservation of energy: energy can be transferred and transformed, but it is neither created nor destroyed.